Chemistry Chapter 3 Summary Flashcards
How does ionic bonding work
Electrons are transferred to form ions with full outer shells of electrons
What does ionic bonding occur between
Metals and non-metals
How are ions in ionic compounds held together
In giant lattice structures by electrostatic forces
Why do ionic compounds have very high melting and boiling points
The electrostatic forces are very strong and need a lot of energy to break apart
Why can melted or dissolves ionic compounds conduct electricity
The ions are free to move
What type of atoms form covalent bonds
Non-metals
Why do simple covalent structures have low melting and boiling points
The intermolecular forces are very weak
Why don’t simple molecules conduct electricity
They have no free ions or electrons
Why do bigger molecules have higher melting and boiling points
They have stronger intermolecular forces
Why is diamond so much stronger than graphite
In diamond the carbon atoms form four covalent bonds, creating a solid lattice with no free electrons while in graphite the carbon only form three covalent bonds creating sheets of carbon atoms arranged in hexagons with the sheets held together by weak intermolecular forces, making graphite much weaker than diamond.
